Answered: the concentration of H3O+

Science

Chemistry

the concentration of H3O+

General, Organic, and Biological Chemistry

7th Edition

ISBN:9781285853918

Author:H. Stephen Stoker

Publisher:H. Stephen Stoker

Chapter10: Acids, Bases, And Salts

Section: Chapter Questions

Problem 10.104EP: Both ions in the salt ammonium acetate (NH4C2H3O2) hydrolyze in aqueous solution. Explain why this...

See similar textbooks

Related questions

Q: Calculate the hydronium-ion concentration at 25°C in a 1.2 x 10-2 M Ba(OH)2 solution. Concentration…

A: Given- Concentration of Ba(OH)2 solution = 1.2 x 10-2 M To find- Hydronium ion concentration =…

Q: Which of the following solutions has the highest concentration of H+ ions: 0.35 M HCl, 0.25 M H2SO4,…

A: Let's classify given compounds into strong /weak acids. Strong acid - HCl , H2SO4 Weak acid - H3PO4…

Q: 0.1 M NH4CI solution, using the given pH data, write net-ionic equation for hydrolysis: NH4* + H20 +…

A: Salt hydrolysis :- The interaction of cation or anion or both of a salt to form an acidic or basic…

Q: Arsenic acid has a Ka1 of 5.6x10-3, Ka2 of 1.0x10-7, and Ka3 of 3.0x10-12, 1) Identify the acid as…

A: It is triprotic acid, it gives three protons. The pH of the arsenic acid will be around 1.19 Please…

Q: Which of the following solutions of monoprotic acids has the HIGHEST concentration of its conjugate?…

A: Acid and conjugate base For an acid HA, HA(aq)+H2O(l)→A-(aq)+H3O+(aq) The equilibrium constant is :…

Q: For H3PO3, Ka1= 4.06x10^-2 and Ka2= 3.92x10^-7. Calculate the pH of 0.295 molar solution H3PO3

Q: A 0.21-mol sample of a diprotic acid, H2A, is dissolved in 250 mL of water. The Ka1 of this acid is…

A: Given that: Moles of diprotic acid, H2A = 0.21 mol Volume = 250 mL = 0.250 L (use 1 L = 1000 mL)…

Q: Carbonic acid, H2CO3, is a diprotic acid with Ka1 = 4.2 x 10-7 and Ka2 = 4.7 x 10-11. Calculate the…

A: It is given that H2CO3 is a diprotic acid, and has Ka1 = 4.2×10-7 and has Ka2 = 4.7×10-11, and the…

Q: A solution is contaminated with traces of copper, nickel, and zinc. Which option would be the safest…

A: Given: A solution with traces of copper, nickel and zinc. To describe the safest way to make it…

Q: The percent ionization of niacin 1Ka = 1.5 x 10-52 in a 0.020M solution is 2.7%. Calculate the…

Q: What volume (mL) of 0.201 M potassium hydroxide (KOH) will it take to reach the equivalence point in…

Q: Calculate the concentrations of ALL the ions present in a 0.0300M solution of carbonic acid (H2CO3…

A: H2CO3 is a weak acid. It is form from the reaction of CO2 with water. Given data: Ka1 = 4.2×10-7…

Q: The molar concentration of hydroxide ion in pure water at 25 °C is ________. A) 1.00 B) 0.00 C) 1.0…

Q: A 4.5x10^-3M solution of a weak acid is 6.3% dissociated at 25°C. In a 4.5x10^-4 M solution, the…

Q: What is [H30+] in a solution of 0.25 M CH3CO2H and 0.030 M NaCH3CO2? CH3CO,H(aq) + H20(1) = H30*(aq)…

A: Acetic acid and sodium acetate form buffer solution

Q: solution is prepared that contains 0.2 M HNO3 and 0.1 M HN3 (Ka=1.9x10-5). What is the concentration…

Q: What is the pH of a 0.10 M H2C2O4 solution that has the stepwise dissociation constants Ka1 = 5.9 ×…

Q: A 50.00-mL portion of an HCl solution required 29.71 mL of 0.01963 M Ba(OH)2 to reach an end point…

A: Given: The volume of HCl solution = 50.00 mL = 0.050 L The volume of Ba(OH)2 (barium hydroxide) =…

Q: you mix together 50.0 mL of 0.25 M (NH4)2S and 50.0 mL of 0.20 M NH4Cl. What will the resulting…

Q: What is the hydronium-ion concentration of a 0.25 M solution of HCN (Ka = 4.9 × 10–10) at 25°C?

A: Given, Ka = 4.9×10-10 pka = -log(Ka) = -log(4.9×10-10) = 9.31 Concentration of Acid (C) = 0.25 M…

Q: Calculate the [H+], [H2PO4-], [HPO4-2], [PO4-3] and [H3PO4] in a 0.10 M solution of phosphoric acid.…

A: Answer:

Q: Given for H2X: Kat = 4.5 x 10; Ka2 = 1.2 x 10 1 The concentration of X "in a 0.150 M aqueous…

A: Given, First acid dissociation constant of diprotic acid H2X = Ka1 = 4.5 x 10-2 Second acid…

Q: Calculate the molar H3O+ ion concentration of a solution if the OH- ion concentration is (a)…

Q: Sample Color Indicator Nature 1. Tap Water Pale Blue 2. Distilled Water Pale Violet 3. Baking Soda…

Q: he pH of the solution formed by mixing 50 ml of 0.1 M CH3COOH solution (Ka = 1.8 × 10-⁵) with 45 ml…

A: Answer :- (b) 5.7 The pH of the solution formed by mixing 50 ml of 0.1 M CH3COOH solution (Ka =…

Q: Calculate the concentrations of hydronium ion and hydroxide ion at 25°C in: 0.11 M HNO3 [H3O+]…

A: We know that strong acid or base dissociates completely in water. So if we consider the case of…

Q: With the use of ICE, calculate the % ionization of the solute in 0.1M HNO2 solution. Ka =…

A: Percent ionization is given by the expression, α=Kac×100%

Q: How to prepare 50 ml. 1x PBS solution (pH 7.4).

A: Phosphate Buffered Saline (PBS) : Phosphate Buffered Saline is an isotonic buffer, which is…

Q: %3D What is the pH of a 0.1000 M NACH3COO solution? (Ka CH3COOH = 1.8x10^-5) 4.75 5.13 8.87 7.45…

A: We have find out pH of 0.1000 MNaCH3COO Solution.

Q: A solution of dimethylamine is prepared by dissolving 1.3525 grams of dimethylamine in 25 mL ethanol…

A: Dimethylamine reacts with HCl as: CH3NHCH3+HCl→CH3NH2+CH3+Cl-

Q: How many grams of ascorbic acid and mL of 0.1M sodium hydroxide must be added to 100 mL of water to…

A: Given: Concentration of NaOH = 0.1 M pH = 3.9 Total concentration = 0.25, 0.5, and 0.1mM ka of…

Q: phenolphthalein is an indicator that when added to a soltuion, appears clean at a ph belowe 8 and…

A: Given Phenolphthalein is an indicator that when added to a solution, appears clean at a pH below 8…

Q: 1. Calculate the pH of each solution. a. [H*] = 5.0 x 10-6 M b. [H] = 8.3 x 10-1⁰ M c. [H*] =2.7 x…

Q: A 50.0 mL sample may contain the following compounds, alone or in some combination, along with inert…

A: 50 ml sample contains mixture of acids along with inert materials. We are using two indicators. We…

Q: Calculate the concentration of C8H.O42 : a. in a solution which is 0.020 M solution of H2C8H4O4. b.…

Q: What is the approximate pH of a solution formed by mixing 45.0 mL of 0.10M HNO3, 50.0 mL of 0.20M…

A: Given: The volume of HNO3=45.0 mL Molarity of HNO3=0.10M Volume of HCl=50.0 mL Molarity of…

Q: Which pH would change the least if each of the following were diluted by adding

A: The correct answer is C

Q: Calculate the concentration of free Ca2 in a solution of 0.10 M CaY2 at pH 6. K for CaY2 is 4.9x1010…

Q: Calculate how much of each solution you need to take to prepare 1 L of buffer solution with a pH of…

A: The question deals with the concept of Buffer preparation. by adding suitable amount of sodium…

Q: Calculate [A-] and [A2-]of a 0.010 M solution of diprotic acid, H2A, with K1 = 1.1 x 10-3 and K2 =…

A: Given, K1 = 1.1 x 10-3 K2 = 3.5 x 10-7 [H2A]=0.010 M

Q: Determine the percent ionization of a 3.75 MHClO solution. Ka =2.9 x 10-8

Q: Calculate the concentration of bicarbonate ion, HCO3-1, in a 0.010 M H2CO3 solution that has the…

A: The dissociation constant represents the tendency of a chemical substance for reversible…

Q: The Ka of formic acid is 1.78x10-4. Compute the resulting pH of a 0.100 M solution of formic acid…

A: Since you have posted a question with multiple subparts, we will solve the first three subparts for…

Q: Calculate the percent dissociation of a 0.085 M solution of acetic acid, HC2H302. (ka=1.9x10)…

A: Formula to calculate dissociation constant :

Q: Calculate the hydronium-ion concentration at 25°C in a 1.3 x 10-2 M Ba(OH)2 solution. Concentration…

A: The Ba(OH)2 dissociates in solution as- Ba(OH)2 (aq)→Ba2+(aq) + 2OH-(aq) Thus, as per balanced…

Q: Calculate the concentrations of H30*, OH and Cl" in a 0.20 M aqueous solution of HCI. O a. [H3O*] =…

A: In this question, concentrations of H3O+ , OH- and Cl- in a 0.20 M aqueous solution of HCl is to be…

Q: Calculate the percent dissociation of 4-chlorobutanoic acid (C3H CICO₂H) in a 4.9M aqueous solution…

A: We would write dissociation equation of 4-chlorobutanoic acid as use its Kb value .

Concept explainers

Ionic Equilibrium

Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.

Arrhenius Acid

Arrhenius acid act as a good electrolyte as it dissociates to its respective ions in the aqueous solutions. Keeping it similar to the general acid properties, Arrhenius acid also neutralizes bases and turns litmus paper into red.

Bronsted Lowry Base In Inorganic Chemistry

Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.

Question

100%

Calculate the concentration of H3O+, H2AsO4-, HAsO4-2, AsO4-3 and H3AsO4 in a solution of 0.3M H3AsO4. Ka1= 2.5x10^-4 Ka2= 5.6x10^-8 Ka3= 3x10^-13

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Step by step

Solved in 2 steps with 2 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

A 0.21-mol sample of a diprotic acid, H2A, is dissolved in 250 mL of water. The Ka1 of this acid is 1.0 × 10–5 and Ka2 is 1.0 × 10–10. Calculate the concentration of A2– in this solution. 1) 1.0 × 10–5 M 2) 1.4 × 10–3 M 3) 2.9 × 10–3 M 4) 1.0 × 10–10 M 5) 0.84 M
The percent ionization of niacin 1Ka = 1.5 x 10-52 in a 0.020M solution is 2.7%. Calculate the percentage of niacin moleculesionized in a solution that is (a) 0.010 M, (b) 1.0 x 10-3 M.
Calculate the PH of a solution made by mixing 50 ml of 0.3 M citrate monobasic with 25 mL of 0.2 M citrate dibasic. Ka1 = 7.1E-4, Ka2 = 1.7E-5, Ka3 = 6.4E-6.
Calculate the [H+], [H2PO4-], [HPO4-2], [PO4-3] and [H3PO4] in a 0.10 M solution of phosphoric acid. Ka1 = 7.5 x 10-3 Ka2 = 6.2 x 10-8 Ka3 = 1.0 x 10-12
Calculate the concentration of the carbonate and bicarbonate ion in one sample. (Ka2 H2CO3 is 4.7 x 10-11) using the equation [alkalinity] = 2[CO3 2- ] + [HCO3 - ] + [OH- ] – [H30 + ] pH = 8.10 alkalinity = 135.8mg/L
What volume (mL) of 0.201 M potassium hydroxide will it take to reach the equivalence point in a 16.3 mL aliquot of 0.226 M triprotic acid? A) 2.22 B) 18.3 C) 55.0 D) 6.11
Determine the pH of a solution made of 0.0082M H3PO4 and 0.0046M Na2HPO4. (Ka of H3PO4 = 7.11 x 10-3)
What is the pH of a 0.10 M H2C2O4 solution that has the stepwise dissociation constants Ka1 = 5.9 × 10-2 and Ka2 = 6.4 × 10-5?
What is the concentration of X2– in a 0.150 M solution of the diprotic acid H2X? For H2X, Ka1 = 4.5 x 10–6 and Ka2 = 1.2 x 10-11. 9.9 x 10-8M 2.0 x 10-9 M 8.2 x 10-4 M 1.2 x 10-11M
What is the pH of a solution that is 0.125 M in maleic acid, a DIPROTIC acid with Ka1=1.2x10-2 and Ka2=4.7x10-7.
The Kb of HONH2 is 1.1x10^-8 a. calculate the pH and percent dissociation of a solution containing 0.100M HONH2. b. calculate the pH and percent dissociation of a mixture containing 0.100 M HONH2 and 0.100M HONH3Cl
what is the pH of a solution prepared by mixing 50.0 mL of 0.125 M amonia and 25.0 mL of 0.100 M hyrogen chloride (The acid dissociation constant of amonnium ion is 5.70x10-10)